Test Chapter ATOMIC STRUCTURE
Subject: Chemistry Total
Marks: 25
Class: XI Max
time: 60 minutes
- Write the difference between emission spectrum and absorption spectrum. (1)
- Why the energy of electron in an atom is negative? (1)
- What is Hund’s rule of maximum multiplicity? Explain with examples. (1)
- Two electrons occupy the same orbital together despite the repulsions of like electrostatic charges. (1)
- Write the complete symbol for the atom with the given atomic number
(Z) and atomic
mass (A).
(a) Z
= 17 A = 35
(b) Z =
4 A = 9 (1)
6. Which of the following ions are unlikely and Why? K+ and
I3- (1)
7. Explain why the electronic configuration of Cr is [Ar] 3d54s1
and not [Ar]
3d44s2 (1)
8. State Pauli’s exclusion principle. (1)
9. Calculate the total number of electrons
present in 2g of CH4. (2)
10. Write the
differences between cathode rays and anode rays. (2)
11. Calculate
the wave number of the line of frequency 4 x 1014 s-1 (2)
12. Write the
main postulates of Planck’s Quantum theory. (2)
13. If the
velocity of electron in Bohr’s first orbit is 2.19 x 108 m/s.
Calculate the
de- Broglie wavelength associated with it. (2)
14. Explain line spectrum of
Hydrogen. (2)
15. Using s, p, d notations,
describe the orbital with the following
quantum numbers.
a)
n = 1, l = 0
b)
n = 3, l = 1
c)
n = 4, l = 2
d)
n = 4, l = 3 (2)
16. (i) An atomic orbital has n
= 3. What are possible values of l and ml ?
(ii)
List the quantum numbers (ml and l) of electrons for 3d orbital. (3)
(iii)
Which of the following orbitals are possible?
1p,
2s, 2p and 3f
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